Name: finding kc from equilibrium data
Uploaded: 2020-09-24T15:06:50.000Z
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Chemistry

Matter and its Interactions

PS.Chm.5.2

Calculating the Equilibrium Constant

La constante d'équilibre, Kc, peut être déterminée en remplaçant les valeurs correspondantes dans l'expression constante d'équilibre si les concentrations de tous les réactifs et produits à l'équilibre sont connus. Un mélange gazeux de dioxyde de soufre et d'oxygène à 530 degrés Celsius peut réagir selon la réaction indiquée. A l'équilibre, le mélange contient 0, 10 molaire de dioxide de soufre, 0, 15 molaire d'oxygène et 10, 88 molaire de soufre trioxyde.En substituant les valeurs dans l'expression d'équilibre, le Kc est égal à 7, 9 10⁴. Le Kc peut également être calculé à condition que la concentration initiale de tous les composants et la concentration d'équilibre d'au moins un composé est connu. Les concentrations d'équilibre inconnues peuvent alors être calculés en utilisant la stoechiométrie réactionnelle.Le tableau ICE est utilisé pour organiser les informations relatives aux concentrations initiales, de changement et d'équilibre de la réaction. Lorsqu'on laisse un mélange réactionnel contenant 0, 11 molaire d'azote et 0, 36 molaire d'hydrogène atteindre l'équilibre à 500 degrés Celsius, il produit 0, 020 molaire d'ammoniac à l'équilibre. Pour calculer le Kc, les concentrations d'équilibre de l'azote et de l'hydrogène doivent être déterminés.La stœchiométrie de la réaction montre que 1 mole d'azote gazeux et 3 moles d'hydrogène gazeux sont nécessaires pour produire 2 moles de gaz ammoniac. Le changement, x, multiplié par les coefficients des réactifs et des produits, désigne la concentration des réactifs consommés et la concentration du produit fabriqué pour atteindre l'équilibre. Puisque 2x est égal à 0, 020, x est égal à 0, 010.La concentration d'équilibre d'azote et d'hydrogène peut alors être déterminée en soustrayant le changement de concentration respectif à partir de leur concentration initiale qui est égale à 0, 10 et 0, 33 molaire, respectivement. En substituant les concentrations à l'équilibre dans l'expression du Kc le Kc est égal à 0, 11. Le Kp des réactions impliquant des gaz peut être calculé à l'aide d'une tableau ICE et de l'expression de l'équilibre écrite avec des pressions partielles.

calcul de la constante d'équilibre

La constante d'équilibre d'une réaction est calculée à partir des concentrations (ou pressions) à l'équilibre de ses réactifs et produits. Si ces concentrations sont connues, le calcul implique simplement leur substitution dans l'expression de Kc. 
 Par exemple, le dioxyde d'azote gazeux forme du tétraoxyde de diazote selon cette équation : 
 <img alt="Eq1" src="/files/ftp_upload/11388/11388_Equation_1.png" style="text-align: center; height: 50px;" />
 Lorsque 0,10 mol de NO2 est ajouté à une fiole de 1,0 L à 25 °C, la concentration change de sorte qu'à l'équilibre, [NO2] = 0,016 M et [N2O4] = 0,042 M. La valeur de la constante d'équilibre pour la réaction peut être calculée comme suit : 
 <img alt="Eq2" src="/files/ftp_upload/11388/11388_Equation_2.png" style="text-align: center; height: 90px;" />
 Un exemple un peu plus difficile est fourni ensuite, dans lequel la stœchiométrie de la réaction est utilisée pour déduire les concentrations à l'équilibre à partir des informations fournies. La stratégie de base de ce calcul est utile pour de nombreux types de calculs d'équilibre et repose sur l'utilisation de termes pour les concentrations de réactif et de produit initialement présentes, pour la façon dont elles changent au fur et à mesure que la réaction se produit, et pour ce qu'elles sont quand le système atteint l'équilibre. L'acronyme ICE est couramment utilisé pour faire référence à cette approche mathématique, et les termes de la concentration sont généralement rassemblés sous un format tabulaire appelé un tableau ICE. 
 Calcul d'une constante d'équilibre 
 Les molécules d'iode réagissent de façon réversible avec les ions iodure pour produire des ions triiodure. 
 <img alt="Eq3" src="/files/ftp_upload/11388/11388_Equation_3.png" style="text-align: center; height: 50px;" />
 Si une solution ayant des concentrations de I2 et de I− toutes deux égales à 1,000 × 10−3 M avant la réaction donne une concentration à l'équilibre pour I2 de 6,61 × 10−4 M, quelle est la constante d'équilibre de la réaction ? 
 Pour calculer les constantes d'équilibre, les concentrations à l'équilibre sont nécessaires pour tous les réactifs et produits : 
 <img alt="Eq4" src="/files/ftp_upload/11388/11388_Equation_4.png" style="text-align: center; height: 90px;" />
 Les concentrations initiales des réactifs et la concentration à l'équilibre du produit sont fournies. Ces informations peuvent être utilisées pour calculer les termes des concentrations à l'équilibre des réactifs, en présentant toutes les informations dans un tableau ICE. 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;"></td>
 <td style="color: black; border: 1px solid black; text-align: center;">    I2 (aq)         </td>
 <td style="color: black; border: 1px solid black; text-align: center;">I− (aq) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">   I3− (aq)    </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentration initiale (M) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">1,000 × 10−3 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">1,000 × 10−3 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">0 </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Changement (M) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">−x </td>
 <td style="color: black; border: 1px solid black; text-align: center;">−x </td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentration à l'équilibre (M) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">  1,000 × 10−3 − x   </td>
 <td style="color: black; border: 1px solid black; text-align: center;">    1,000 × 10-3 − x   </td>
 <td style="color: black; border: 1px solid black; text-align: center;">x </td>
 </tr>
 </tbody>
 </table>
 À l'équilibre, la concentration de I2 est de 6,61 × 10−4 M donc 
 <img alt="Eq5" src="/files/ftp_upload/11388/11388_Equation_5.png" style="text-align: center; height: 90px;" />
 Le tableau ICE peut maintenant être mis à jour avec des valeurs numériques pour toutes ses concentrations : 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;"></td>
 <td style="color: black; border: 1px solid black; text-align: center;">I2 (aq)  </td>
 <td style="color: black; border: 1px solid black; text-align: center;">I− (aq) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">I3− (aq) </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentration initiale (M) </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> 1,000 × 10−3  </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> 1,000 × 10−3   </td>
 <td style="color: black; border: 1px solid black; text-align: center;">0 </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Changement (M) </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> −3,39 × 10−4  </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> −3,39 × 10−4   </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> +3,39 × 10-4  </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentration à l'équilibre (M) </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> 6,61 × 10−4  </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> 6,61 × 10−4   </td>
 <td style="color: black; border: 1px solid black; text-align: center;"> 3,39 × 10−4  </td>
 </tr>
 </tbody>
 </table>
 Enfin, les concentrations à l'équilibre peuvent être substituées dans l'expression de Kc et résolues : 
 <img alt="Eq6" src="/files/ftp_upload/11388/11388_Equation_6.png" style="text-align: center; height: 90px;" />
 Ce texte a été adapté d'<a href="https://openstax.org/books/chemistry-2e/pages/13-4-equilibrium-calculations">Openstax, Chimie 2e, Section 13.4 Calculs d'équilibre</a>.

Calcul de la constante d'équilibre

La constante d’équilibre d’une réaction est calculée à partir des concentrations d’équilibre (ou pressions) de ses réactifs et produits. Si ces ...

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Chemical Equilibrium

Équilibre chimique

KEY TERMS AND CONCEPTS

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finding kc from equilibrium data

The equilibrium constant, Kc, can be found from the equilibrium concentrations of reactants and products. When those concentrations are known, the calculation is straightforward. The values are placed into the Kc expression for the reaction.

One example uses nitrogen dioxide and dinitrogen tetroxide. When 0.10 mol NO2 is added to a 1.0-L flask at 25 °C, the concentrations change until equilibrium is reached. At equilibrium, [NO2] is 0.016 M and [N2O4] is 0.042 M, and these values are used to calculate the equilibrium constant for the reaction.

A more advanced example uses reaction stoichiometry to find equilibrium concentrations from the information given. This method is useful for many equilibrium calculations. It tracks the amount present at the start, how it changes as the reaction proceeds, and the amount present at equilibrium. The acronym ICE is used for this approach, and the values are often organized in an ICE table.

The iodine example shows how this works. I2 reacts reversibly with iodide ions to form triiodide ions. If a solution starts with 1.000 × 10^-3 M I2 and 1.000 × 10^-3 M I−, and the equilibrium concentration of I2 is 6.61 × 10^-4 M, the equilibrium constant can be found for the reaction.

To do this, the initial concentrations of the reactants and the equilibrium concentration of the product are used to build an ICE table. The table shows I2, I−, and I3− with initial, change, and equilibrium entries. From the given equilibrium value for I2, the other concentrations can be calculated, including 6.61 × 10^-4 M for I2 and I− and 3.39 × 10^-4 M for I3−.

Once the equilibrium concentrations are known, they are substituted into the Kc expression and solved. This same strategy links the ICE table to the final equilibrium constant. It is a practical way to handle equilibrium problems in chemistry.

Finding Kc from Equilibrium Data

the equilibrium constant

Chemical Equilibrium and Kc Rules

Chemical equilibrium and the equilibrium constant Kc describe how reactants and products are balanced in a reaction. In the oxidation of sulfur dioxide, a mixture that starts with reactants only has no product at first. As the reaction moves forward toward equilibrium, reactant concentrations decrease and product concentration increases. When equilibrium is reached, the concentrations of both stay constant. A reaction can also begin with only products present. In that case, the reaction moves...

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homogeneous-equilibria-for-gaseous-reactions

Relating Kc and Kp in Gas Equilibria

Gas-phase equilibrium can be written using either concentration or pressure. The equilibrium constant may be shown as Kc, which uses molar concentration, or as Kp, which uses partial pressure of the reactants and products. The link between Kc and Kp comes from the ideal gas equation and the definition of molarity. Molarity is the number of moles divided by volume. In the ideal gas equation, P stands for partial pressure, V for volume, n for number of moles, R for the gas constant, and T for...

le chatelier's principle: changing concentration

le-chatelier-s-principle-changing-concentration

Shifting Equilibrium by Changing Concentration

Chemical equilibrium is a dynamic balance. At equilibrium, the forward and reverse reactions happen at equal rates. If the system is stressed in a way that changes one rate more than the other, it is no longer at equilibrium and will shift until balance is restored. This behavior is described by Le Châtelier’s principle. Changes in concentration are a major stress on an equilibrium system. Reaction rates depend mainly on concentration and temperature. For that reason, changing the amount of a...

calculating the equilibrium constant

The equilibrium constant, Kc, can be found from the equilibrium concentrations of reactants and products. When those concentrations are known, the calculation is straightforward. The values are placed into the Kc expression for the reaction. One example uses nitrogen dioxide and dinitrogen tetroxide. When 0.10 mol NO2 is added to a 1.0-L flask at 25 °C, the concentrations change until equilibrium is reached. At equilibrium, [NO2] is 0.016 M and [N2O4] is 0.042 M, and these values are used to...

reaction quotient

Using Q to Track Equilibrium Changes

Reaction quotient Q helps track how far a reversible reaction has moved toward equilibrium. For a balanced reaction such as m A + n B ⇌ x C + y D, Q comes directly from the stoichiometric coefficients in the equation. When concentrations are used, the expression is written as Qc. For gases, a similar form uses partial pressures. These expressions use relative concentration and pressure values, not absolute values. That means reaction quotients are dimensionless and have no units. As a reaction...

dynamic equilibrium

Chemical Equilibrium in Reversible Reactions

Chemical equilibrium in reversible reactions happens when a reaction moves in both directions at the same time. A reversible reaction uses a double arrow to show that products can turn back into reactants. At equilibrium, the concentrations of reactants and products stay constant over time because the forward and reverse reaction rates are equal. The video uses the reversible decomposition of colorless dinitrogen tetroxide to brown nitrogen dioxide as an example. At time zero, there is finite...

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Equilibrium Concentrations from an ICE Table

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le chatelier's principle: changing volume (pressure)

le-chatelier-s-principle-changing-volume-pressure

Gas Equilibrium Under Volume Changes

Gas-phase equilibrium can shift when the volume of the system changes. In these reactions, a change in pressure changes concentration because the partial pressure of an ideal gas is proportional to its molar concentration. That means pressure changes affect equilibrium in the same way as concentration changes. When the volume of a gas mixture changes, the concentrations of reactants and products change together. Since every gas in the equilibrium occupies the same space, the same volume change...

le chatelier's principle: changing temperature

le-chatelier-s-principle-changing-temperature

Le Chatelier's Principle in Heating and Cooling

Le Chatelier's principle helps explain how chemical equilibrium responds to heating and cooling. A system at equilibrium will shift to restore balance after a temperature change, but the equilibrium constant, K, will not stay the same. Instead, the mixture reaches a new equilibrium with a different composition. This temperature effect is different from a concentration change, which shifts equilibrium without changing K. To understand why temperature matters, the reaction can be written with...

the small x assumption

Estimating Equilibrium with Small Changes

A small equilibrium constant can make equilibrium calculations easier. In these reactions, the equilibrium position favors the reactants. When the initial reactant concentration is high and the Kc value is small, the change in concentration may be negligible. In that case, the equilibrium concentration is close to the initial concentration. This idea helps simplify weak acid and weak base problems. Chemists can assume that some equilibrium concentrations are equal to the initial concentrations.

key terms and concepts

Use equilibrium concentrations and ICE tables to find Kc in chemistry. See how nitrogen dioxide and iodine examples connect data to the equilibrium constant.

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Finding Kc from Equilibrium Data

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